Ready to sharpen your titration skills? Our Ultimate Titration Practice Problems Quiz is designed for students and lab enthusiasts eager to master acid-base titration. With free titration practice problems, you'll tackle sample titration problems and chem titration problems that simulate real lab scenarios. Wondering how precise your calculations are? These titration practice questions guide you step by step, from preparing a buffer solution to performing a perfect titrimetric test . Whether you're new to acid-base chemistry or reviewing for exams, enhance your skills with our acids and bases quiz . Jump in, challenge yourself, and celebrate each success. Let's get started - take the quiz now and watch your confidence in titration soar!
What is the equivalence point in a titration?
The initial point of titration
The point where moles of acid equal moles of base
When half the acid has been neutralized
The moment the indicator first changes color
The equivalence point is reached when stoichiometrically equivalent amounts of acid and base have reacted, meaning moles of H+ = moles of OH?. It is not the initial or half-neutralization point, nor simply when an indicator begins to change. At this point, titrant and analyte are in perfect stoichiometric balance. For more details on equivalence point concepts, see Chemguide on titrations.
Which indicator is most suitable for a strong acid - strong base titration?
Phenolphthalein
Cresol red
Bromocresol green
Methyl orange
Phenolphthalein changes color in the pH range 8.2 - 10.0, which covers the steep portion of the titration curve for a strong acid vs. strong base. While other indicators have different transition ranges, phenolphthalein gives a clear endpoint for this type of titration. Methyl orange, for example, works best in acidic endpoints. See Chemguide on indicators.
In the titration equation M?V? = M?V?, what does M represent?
Moles (mol)
Volume (L)
Molarity (mol/L)
Mass (g)
In the dilution and titration relationship M?V? = M?V?, M? and M? represent the molarities (concentrations) of the two solutions. Volume (V) units must be consistent, and this formula directly relates how concentration and volume change in a titration. For more, visit LibreTexts on titration calculations.
What is the pH at the equivalence point when titrating a strong acid with a strong base?
Greater than 7
Depends on the indicator
Less than 7
7.00
A strong acid - strong base titration reaches a neutral solution at equivalence because the conjugate acid and base are both non?significant in terms of pH. Thus the pH is 7.00 at 25 °C. This is independent of the indicator choice. See Khan Academy on titration curves.
Which of the following is a suitable indicator for titrating a weak acid with a strong base?
Litmus paper
Methyl orange
Phenolphthalein
Bromothymol blue
Phenolphthalein has a transition range around pH 8.2 - 10.0, which overlaps the equivalence point (pH > 7) of a weak acid with a strong base. Methyl orange and bromothymol blue have ranges too acidic or too neutral for clear endpoints. More on indicator selection at Chemguide.
What volume of 0.10 M NaOH is required to neutralize 25.00 mL of 0.10 M HCl?
50.00 mL
Insufficient information
10.00 mL
25.00 mL
Using M?V? = M?V?, (0.10 M)(25.00 mL) = (0.10 M)(V?) gives V? = 25.00 mL. Equal molar solutions require equal volumes for neutralization. For more practice, see LibreTexts on Molarity and Titration.
What does normality (N) represent in titration calculations?
Liters per mole
Grams per liter
Moles per liter
Equivalents per liter
Normality is defined as the number of chemical equivalents (acid or base equivalents) per liter of solution. It is used in titrations to account for multiple reactive sites per molecule. More on normality is available at Chemguide on normality.
Which of the following best describes the endpoint of a titration?
The pKa of the acid equals the pH
The equivalence point
When the indicator changes color
When half the acid is neutralized
The endpoint is the experimental signal that the equivalence point has been reached, most commonly the color change of an indicator. It may not exactly coincide with the theoretical equivalence point but is a practical approximation. Further details at Khan Academy.
What is the pH at the halfway point of a weak acid titration?
Less than 7
Greater than 7
7.00
Equal to pKa
At the half?neutralization point, [HA] = [A - ], so by the Henderson - Hasselbalch equation pH = pKa + log([A - ]/[HA]) = pKa. This holds true for any monoprotic weak acid titration. See Chemguide on Henderson - Hasselbalch.
During titration of a weak acid HA with NaOH, the solution at equivalence point contains primarily:
A - and water
HA and excess OH -
H+ and A -
Pure water
At the equivalence of HA + OH - , the acid is fully converted to its conjugate base A - and water. The conjugate base hydrolyzes, giving a basic pH. Visit LibreTexts on titration curves for more.
How many moles of HCl are present in 0.250 L of 2.00 M HCl?
2.50 mol
5.00 mol
0.125 mol
0.500 mol
Moles = Molarity × Volume = 2.00 mol/L × 0.250 L = 0.500 mol. This straightforward calculation is fundamental to preparing titration solutions. See Khan Academy on moles and molarity.
During the titration of a diprotic acid H2A with NaOH, how many distinct equivalence points are observed?
2
1
Depends on Ka values
3
A diprotic acid donates two protons in two separate steps, each with its own equivalence point. Thus, you observe two jumps in the titration curve. More on polyprotic titrations at Chemguide on polyprotic acids.
Which indicator is most suitable for titrating a weak base with a strong acid?
Universal indicator
Phenolphthalein
Thymol blue
Methyl orange
Methyl orange transitions at pH 3.1 - 4.4, which overlaps the acidic equivalence point (pH < 7) of a weak base - strong acid titration. Phenolphthalein would change too late. More details at Chemguide on choosing indicators.
If 40.0 mL of 0.100 M NaOH completely neutralizes 20.0 mL of an acid, what is the acid's concentration?
0.200 M
0.050 M
0.100 M
0.400 M
M?V? = M?V? ? Madid × Vadid = Manc × Vanc ? (0.100 M)(0.040 L) = Macid × 0.020 L, so Macid = 0.200 M. This method is standard for titration calculations. See LibreTexts Quantitative Analysis.
What buffer system is formed when equal moles of acetic acid and sodium acetate are mixed?
Ammonia/ammonium buffer
Phosphate buffer
Carbonic acid/bicarbonate buffer
Acetic acid/acetate buffer
A buffer contains a weak acid and its conjugate base in appreciable quantities. Equal moles of acetic acid (CH?COOH) and acetate (CH?COO - ) create an acetic acid/acetate buffer at pH ? pKa. More on buffer solutions at Khan Academy.
Which term describes the point on a titration curve where the pH changes most rapidly?
Buffer region
Equivalence point
Endpoint
Half-equivalence point
The equivalence point corresponds to the steepest part of the titration curve, where a small addition of titrant causes a large pH change. The endpoint is the experimental detection, which may slightly differ. Read more at LibreTexts on titration curves.
Calculate the pH at the equivalence point when titrating 0.100 M acetic acid (Ka = 1.8×10??) with strong base.
7.00
8.72
6.30
5.12
At equivalence, [A - ] = initial acid moles/total volume ?0.100 M. Kb = Kw/Ka = 1e - 14/1.8e - 5 = 5.56e - 10. pOH = ½(pKb - log C) ? ½(9.25 - ( - 1)) = 5.125, so pH ? 14 - 5.125 = 8.875. Accounting volume change gives ?8.72. See Chemguide titration calculations.
At the half-neutralization point of a diprotic acid titration, which statement is true?
Concentration of H2A equals concentration of HA -
Concentration of HA - equals A2 -
No buffer exists at this point
pH equals second pKa
During the first half?neutralization, H2A has lost one proton, producing HA - , and [H2A] = [HA - ], so pH = pKa?. This region acts as a buffer. More on polyprotic half-equivalence at Chemguide.
In titrating 50 mL of 0.100 M NH3 with 0.100 M HCl, what is the pH after adding 25 mL of HCl?
7.00
5.75
11.50
9.25
At half equivalence for a weak base titration, pOH = pKb so pH = 14 - pKb. For NH?, pKb ? 4.75, so pOH ?4.75 and pH ?9.25. See Henderson - Hasselbalch for bases at LibreTexts.
Which description best matches the titration curve of a weak base with a strong acid?
pH remains constant until endpoint
pH starts high and falls below 7 at equivalence
pH starts low and rises above 7
pH starts at 7 and falls to 0
A weak base solution initially has pH > 7. As strong acid is added, pH gradually decreases, with a steep drop through pH<7 at equivalence due to excess H+. More on titration curves at Khan Academy.
Which factor describes maximum buffer capacity?
[HA] = 0
[A - ] = 0
pH = pKa
pH = 7 always
Buffer capacity is greatest when [HA] = [A - ], which occurs at pH = pKa according to the Henderson - Hasselbalch equation. This allows the solution to resist pH changes most effectively. See Chemguide on buffers.
Where do buffer regions occur in the titration curve of a diprotic acid H2A?
There are no buffer regions in diprotic titrations
Only at the first equivalence point
Only after the second equivalence point
Around each pKa (before and between equivalence points)
Each pKa corresponds to a buffer region where the acid and its conjugate base are both present: around pKa? (before first equivalence) and around pKa? (between first and second equivalence). For more, see LibreTexts on polyprotic acids.
When selecting an indicator, which criterion is most important?
Indicator is the cheapest available
Indicator has the brightest color
Indicator pKa matches titration equivalence pH
Indicator is soluble in organic solvents
An indicator must change color at a pH close to the equivalence point, which means its pKa should lie within the steep section of the titration curve. Cost or color intensity is secondary to matching the pH range. More at Chemguide.
How many milliliters of 0.500 M H2SO4 are needed to neutralize 25.0 mL of 0.500 M Ca(OH)2?
25.0 mL
12.5 mL
75.0 mL
50.0 mL
H2SO4 supplies 2 H+ per molecule and Ca(OH)2 supplies 2 OH - per molecule. Stoichiometry is 1:1 mole H2SO4 to Ca(OH)2, so volumes are equal at the same molarity: 25.0 mL. See LibreTexts on titration stoichiometry.
In titrating 50.0 mL of 0.0500 M H3PO4 (pKa1=2.15, pKa2=7.20, pKa3=12.35) with 0.0500 M NaOH, what is the pH at the second equivalence point?
4.58
7.20
12.29
2.15
At the second equivalence, the predominant species is HPO4²?. Kb for HPO4²? = Kw/Ka3 ?1e - 14/10^( - 12.35)=2.24×10?². [HPO4²?]?0.0025 mol/0.150 L=0.0167 M. pOH?½(pKb - logC)=½(1.65 - ( - 1.78))?1.71, so pH?12.29. See LibreTexts on polyprotic titrations.
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Study Outcomes
Understand acid-base titration fundamentals -
Learn the principles of titration, including equivalence points and indicator selection, to grasp core concepts in acid-base reactions.
Calculate analyte concentrations -
Use titration data to compute unknown solution concentrations through stoichiometric and molarity calculations.
Analyze titration curves -
Interpret titration graphs to identify equivalence points and pKa values, reinforcing data analysis skills.
Apply indicator selection criteria -
Choose appropriate indicators based on titration type and pH range to ensure accurate endpoint detection.
Evaluate experimental errors -
Identify and assess common laboratory mistakes in titrations to improve precision and accuracy.
Cheat Sheet
Equivalence Point vs. Endpoint -
Understanding the equivalence point (when stoichiometric neutralization occurs) versus the endpoint (when your indicator changes color) is crucial for precise titrations. According to MIT OpenCourseWare, the equivalence point is calculated theoretically while the endpoint is an experimental observation. Choose an indicator whose color change closely matches the equivalence pH to minimize titration practice problems errors.
Calculating Molarity with MV = M₂V₂ -
Most titration practice problems use the formula MV = M₂V₂ to relate titrant and analyte concentrations and volumes. For example, if 25.00 mL of 0.100 M NaOH neutralizes 15.00 mL of HCl, then M = (M₂V₂)/V = (0.100×25.00)/15.00 = 0.167 M HCl. Always convert volumes to liters and double-check your unit consistency.
Indicator Selection and pH Curves -
Titration indicators must change color within the steep part of your titration curve, which varies by acid - base strength. Purdue University's chemistry guides show phenolphthalein is ideal for strong-acid/strong-base titrations (pH 8.2 - 10.0) while methyl orange suits strong-acid/weak-base (pH 3.1 - 4.4). Memorize "ph for phenol" to recall that phenolphthalein works in more basic end regions.
Buffer Region & Half-Equivalence Point -
In weak acid or weak base titrations, the midpoint before the equivalence point forms a buffer where pH = pK (Henderson - Hasselbalch equation). At half-equivalence, [HA] = [A❻], so pH = pK, making it easy to find the acid dissociation constant from your titration curve. Reviewing buffer calculations will help you master sample titration problems involving gradual pH changes.
Standardization of Titrants -
Accuracy in chem titration problems starts with a standardized titrant: use a primary standard like potassium hydrogen phthalate (KHP) to determine the exact concentration of NaOH or HCl solutions. Weigh a known mass of KHP and titrate to your chosen endpoint, then calculate molarity via moles = mass/MW. Many university labs (e.g., UC Berkeley) stress this step to ensure reproducible titration practice problems.
